Lead(II) sulfate

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Lead(II) sulfate
sample of lead(II) sulfate
CAS number 7446-14-2 YesY
PubChem 24008
ChemSpider 19956579 YesY
Jmol-3D images Image 1
Molecular formula PbSO4
Molar mass 303.26 g/mol
Appearance white solid
Density 6.29 g/cm3[1]
Melting point 1,087 °C (1,989 °F; 1,360 K)
Solubility in water 0.0032 g/100 mL (15 °C)
0.00443 g/100 mL (20 °C)[2]
Solubility product, Ksp 2.13 x 10-8 (20 °C)
Solubility insoluble in alcohol
Refractive index (nD) 1.877
Crystal structure orthorhombic, barite
heat capacity
103 J/degree mol
Std molar
149 J·mol−1·K−1[3]
Std enthalpy of
−920 kJ·mol−1[3]
EU Index 082-001-00-6
EU classification Repr. Cat. 1/3
Toxic (T)
Harmful (Xn)
Dangerous for the environment (N)
R-phrases R61, R20/22, R33, R62, R50/53
S-phrases S53, S45, S60, S61
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Flash point Non-flammable
Threshold Limit Value 0.15 mg/m3
Related compounds
Other anions Lead(II) chloride, Lead(II) bromide, Lead(II) iodide, Lead(II) fluoride
Other cations Tin(II) sulfate, Sodium sulfate, Copper(II) sulfate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Lead(II) sulfate (PbSO4) is a white crystal or powder. It is also known as fast white, milk white, sulfuric acid lead salt or anglesite.

It is often seen in the plates/electrodes of car batteries, as it is formed when the battery is discharged (when the battery is recharged, then the lead sulfate is transformed back to metallic lead and sulfuric acid on the negative terminal or lead dioxide and sulfuric acid on the positive terminal). Lead sulfate is poorly soluble in water.


Lead(II) sulfate is prepared by treating lead oxide, hydroxide or carbonate with warm sulfuric acid, or by treating a soluble lead salt with sulfuric acid.

Alternatively, it can be produced by the interaction of solutions of lead nitrate and sodium sulfate.


Lead sulfate is toxic by inhalation, ingestion and skin contact. It is a cumulative poison, and repeated exposure may lead to anemia, kidney damage, eyesight damage or damage to the central nervous system (especially in children). Some lead salts may cause reproductive defects and cardiovascular disturbances. It is also corrosive - contact with the eyes can lead to severe irritation or burns. Typical threshold limit value (above which the substance is harmful) is 0.15 mg/m3.


The naturally occurring mineral anglesite, PbSO4, occurs as an oxidation product of primary lead sulfide ore, galena.

Basic and hydrogen lead sulfates[edit]

A number of lead basic sulfates are known: PbSO4·PbO; PbSO4·2PbO; PbSO4·3PbO; PbSO4·4PbO. They are used in manufacturing of active paste for lead acid batteries. A related mineral is leadhillite, 2PbCO3·PbSO4·Pb(OH)2.

At high concentration of sulfuric acid (>80%), lead hydrogensulfate, Pb(HSO4)2, forms.[4]

External links[edit]


  1. ^ "CRC Handbook of Chemistry and Physics", 83rd Edition, CRC Press, 2002.
  2. ^ NIST-data review 1980
  3. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 0-618-94690-X. 
  4. ^ Министерство образования и науки РФ, Реферат "Свинец и его свойства", 2007, http://revolution.allbest.ru/chemistry/00011389_0.html